Chemistry

Chemical Equations - Balanced Chemical Equations (HS-PS1-7)
Chemical Reactions - Determining the Activity Series of Metals
pH Calculations - Calculating pH of a Strong Acid or Strong Base
Nomenclature - Using the Stock Naming System for Ionic Compounds

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HS-PS2-6: Molecular Level Structure of Designed Materials

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Oxidation of Magnesium - Empirical Formula

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This video summarizes an experiment performed to experimentally determine the empirical formula of magnesium oxide. In the lab the mass of a small sample of magnesium ribbon is measured. The metal is then heated in a crucible using a Bunsen burner to speed up the process of oxidation. The reaction forms the product magnesium oxide. The mass of this compound is measured and compared to the original amount of magnesium to determine the added mass of oxygen. The data collected allows students to calculate the empirical formula of the magnesium oxide compound. The reaction is summarized by the following chemical equation. 2Mg  +  O 2  →  2MgO The compound forms with a 1:1 ratio of magnesium to oxygen. This is because magnesium has two valence electrons which are donated to the oxygen atoms. The oxygen atoms can add two electrons to complete their valence shell. I hope this was helpful.
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HS-PS2-5: Magnetic and Electric Fields

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